Inorganic chemistry 3-stage Lec. 2 Dr- leaqaa
Chemical bonds types: Most chemical bonds fall into 2 categories depending on whether the valence e(s) are transferred or shared. Electron in ionic bond are effectively transferred from one atom to another. In covalent bond the e(s) are shared (.) atoms.
1- Ionic bond: - electrostatic forces that exists (.) 2 chemical entities of opposite charge. strongly electropositive elements & nonmetalic,strongly electronegative elements.
* Ionic bond electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl ), charged particles or ions.
CaCl2 Geometry is linear b its most stable electrostatic arrangement.
2-Covalent Bonding Covalent bond: sharing a couple of electrons by the two bonding atoms Its attractive force that exists (.) 2 chemical entities due to sharing a pair of e(s). is type is prevails wn electronegativity differences (.) 2 atoms is not sufficient to produce ions. * inorganic cpds. * prevails in organic chemistry The sharing of the electrons is not always equal between both atoms.
Single Covalent bond *Each molecule a single pair of electrons is shared between the atoms. *homonuclear
COVALENT BONDING Non-polar Covalent The pair of electrons is shared equally by both atoms.(homonuclear) F F, H H, O 2,S8, P4 Polar Covalent The electron pair is not shared equally; the chlorine atom has a greater attraction for the shared electrons than the hydrogen atom. H Cl
The idealistic covalent bonds occur in homonuclear diatomic molecules such as Covalent bonds- Two atoms share one or more pairs of outer-shell electrons.
POLAR COVALENT BONDS when electrons are shared but shared unequally H2O [ water is a polar molecule because oxygen is more electronegative than hydrogen, and therefore electrons are pulled closer to oxygen].
This type of bond is also found as double and triple covalent bonds.
Coordination covalent bond (also donor-acceptor bond) Both bonding electrons provided by one of the atoms (donor), whereas the other atoms provides an empty orbital (akceptor)
3-Coordinate covalent bonding: - covalent interaction but, in this case, both e(s) in the bond arise from a single orbital on one of the atoms forming the bond. (.) complex chemical entities.the entity providing the pair of e(s) is generally referred to as donor species. The acceptor spec. is e(s) deficient and has an empty orbital w can overlap w orbital from the donor.[donor-acceptor complex,coordination cpds]. e.g.complex BF3 etherate This type of bond also occurs in acid-base chemistry (one bond (.) S &O. e.g. oxyacid [sulfuric,nitric chloric &phosphoric acid].
4- Hydrogen bonding: is a 2ry interaction. It as an attractive force that occur (.) certain types of molecules. Wn H is covalent w more electronegative atom such as O,F,N,Cl *association unlike molecule *important role in solution formation & in water crystalization. *H bonding (.) complex molecules & 2ry str. Of proteins,also 2ry binding force in D-R interaction.
5- Van der wals(london) forces Very weak of electrical forces sometimes referred to as induced dipol-induced dipole interactions. Van der waals forces r virtually the only attractive force (.) nonpolar molecules. * association (.) Ar. hydrocarbon molecules such as Benz.(small disturbances in the electrical balance r present in these molecules b of motion of e(s). * nuclear replusion known as van der walls replusion
Coordination (complex) ion ions s central atom of transition metal providing empty orbitals ligands providing free electron pairs Number of ligands (coordination number) is usually 4 or 6 e.g.ferrocyanide
Names of of coordination compounds Names of neutral ligands: H2O aqua NH3 ammin NO nitrosyl CO carbonyl Names of anionic ligands always end in o: F fluoro Cl chloro Br bromo I iodo OH hydroxo CN cyan
Names of of coordination compounds 1. Complex particle is cation: e.g. [Cu(NH3)4]SO4 = Tetraamminecopper(II) sulfate 2. Complex particle is anion: e.g. K3[CoF6] Potassium hexafluorocobaltate(iii)
Werner r theory (the most widely accepted theory of formation complex ion) by Alfred werner (werner complex) *Central metal ion has 2 types of valency: 1-1ry valence(principle valence) (ionizable) [oxidation state on central metal atom] 2-2ry valence(nonionizable): electron pairs [Co(NH3)6]Cl3 1 ry valence = 3 Cl =3, 2 ry valence = 6
*-the ligands r- arranged around metallic ion in certain cc geometry
Ligands: classified according to the number of donor atoms :
Type of ligands: 1- Monodentate ligands :- bond using the electrone pairs of single atom.
- Bidentate ligands bond using the electron pairs of two atoms. -Tridentate ligand Diethylenetriamine (den)
Tetradentate : Triethylenetetramine (trien) Hexadentate ligand EDTA
Octadentate ligand Diethylenetriaminepentaacetate(DTPA) * polydentate ligands are also known as Chelating agents
Polydentate form with metal = ring structure totale # of atoms in ring including metal r- 5,6 or 7. more stable chelate. 4&8-membered rings r- usually unstable
***polydentate ligands used for : chelate forma ----chelating agent [w_ use in pharmaceutical & in drug therapy].